XI Chemistry Chemical Equilibrium Online Test Mdcat-2024

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Instructions for Chapter Chemical Equilibrium Online Test Mdcat-2024:

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    Test Details:

      • Subject: Chemistry
      • Class: 1st year or 11
      • Chapter name: Chemical Equilibrium
      • Test: MDCAT 2024
      • Book: Sindh Textbook
      • Total No. Of MCQS: 50
      • Time Allowed: 50 Minutes
      • Price : Free
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      XI Chemistry Chemical Equilibrium Online Test Mdcat-2024

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      1 / 50

      1. Which of the following best describes a system in chemical equilibrium?

      2 / 50

      2. Which of the following factors does NOT affect the position of equilibrium in a chemical reaction?

      3 / 50

      3. In the equilibrium expression Kc  for the reaction ( aA + bB ⇌  cC + dD ), what does Kc  represent?

      4 / 50

      4. Le Chatelier's Principle states that if a system at equilibrium is disturbed, the system will adjust itself to:

      5 / 50

      5. For the exothermic reaction, N₂(g) + 3H₂ (g) ⇌ 2NH₃ (g)  what effect will increase the temperature have on the equilibrium position?

      6 / 50

      6. Which of the following is a necessary condition for a chemical system to reach equilibrium?

      7 / 50

      7. Which condition is NOT required for a chemical system to achieve equilibrium?

      8 / 50

      8. For the reaction ( aA + bB ⇌cC + dD ), if the concentrations of A and B are increased, what will be the effect on the equilibrium position according to the Law of Mass Action?

      9 / 50

      9. Which of the following best describes the equilibrium constant ( Kc ) for a given reaction?

      10 / 50

      10. According to the Law of Mass Action, what happens to the equilibrium constant ( Kc ) when the temperature of an exothermic reaction is increased?

      11 / 50

      11. In a reaction where the equilibrium constant ( Kc ) is very small, what does this indicate about the reaction?

      12 / 50

      12. The Law of Mass Action can be used to:

      13 / 50

      13. For a given reaction at equilibrium, if the concentration of a product is increased, What will happen according to the Le Chatlier Principal?

      14 / 50

      14. For the reaction ( 2A (g) + B(g) ⇌ 3C (g) ), the equilibrium concentrations are found to be [A] = 0.2M,  [B] = 0.1M, and  [C] = 0.6M. What is the value of the equilibrium constant ( Kc )?

      15 / 50

      15. For the reaction H₂(g) + I₂ (g) ⇌ 2HI (g) ), the initial concentrations are [H₂] = 1M, [I₂] = 1M, and  [HI] = 0M. At equilibrium, the concentration of ( HI ) is 0.8 M. What is the value of ( Kc )?

      16 / 50

      16. Kp>Kc when :

      17 / 50

      17. For the expression : H₂ + I₂ ⇌2HI, unit of Kc will be

      18 / 50

      18. If for a reaction Qc is 2 × 10־² and Kc is 1.3× 10־² then ?

      19 / 50

      19. For a reaction involving gases, what does Delta n represent in the expression ( Kp = Kc (RT)^Δn )?

      20 / 50

      20. If Kp is 5 for a reaction at 300 K and Δn= 1, what is the value of Kc? (Assume ( R = 0.0821 ) L·atm/(mol·K))

      21 / 50

      21. What is the relationship between Kp and Kx  for a reaction involving gases at a constant total pressure?

      22 / 50

      22. Given the reaction ( H₂ (g) + I₂(g)⇌ 2HI (g) ) at equilibrium, if Kc = 50 at 400 K and  Delta n = 0 , what is  Kp ?

      23 / 50

      23. In a chemical reaction, what does it mean if ( Q = Kc )?

      24 / 50

      24. Which of the following statements is true regarding the importance of  Kc  in predicting the extent of a reaction?

      25 / 50

      25. Why is the reaction quotient ( Qc ) useful in predicting the direction of a reaction?

      26 / 50

      26. According to Le Chatelier's principle, what happens to the equilibrium position if the concentration of a reactant is increased?

      27 / 50

      27. For an exothermic reaction, how does an increase in temperature affect the equilibrium position?

      28 / 50

      28. How does an increase in pressure affect the equilibrium of a gaseous reaction where the number of moles of gas decreases?

      29 / 50

      29. What happens to the equilibrium position when a catalyst is added to a reaction?

      30 / 50

      30. In the reaction N₂ (g) + 3H₂ (g) ⇌2NH₃ (g) ), how does decreasing the volume of the reaction vessel affect the equilibrium position?

      31 / 50

      31. For an endothermic reaction, how does a decrease in temperature affect the equilibrium position?

      32 / 50

      32. How does the removal of a product affect the equilibrium position of a reaction?

      33 / 50

      33. In a reversible reaction if certain amount of reactant is added then __ and reaction shift to___

      34 / 50

      34. Select the incorrect statement

      35 / 50

      35. Suitable condition for synthesis of Ammonia:

      36 / 50

      36. The impurities of CaCl₂ and MgCl₂ of brine are removed by treating it with

      37 / 50

      37. What does the solubility product constant Ksp represent?

      38 / 50

      38. Which statement is true regarding the solubility of a salt when a common ion is added to the solution?

      39 / 50

      39. Select the incorrect statement

      40 / 50

      40. If solubility  of BaSO₄ is given then it's Ksp  can be found by:

      41 / 50

      41. Which of the following best illustrates the common ion effect?

      42 / 50

      42. When Ksp>Qsp(Ionic Product) then the solution is said to be

      43 / 50

      43. What is a buffer solution?

      44 / 50

      44. Which of the following is a common example of an acidic buffer solution?

      45 / 50

      45. What is the buffering capacity of a solution?

      46 / 50

      46. Acidic Buffer can be made by mixing of:

      47 / 50

      47. Basic Buffer can be made by mixing of :

      48 / 50

      48. Which of the following is a common application of buffer solutions in biological systems?

      49 / 50

      49. Which buffer system is most commonly used to maintain the pH of blood?

      50 / 50

      50. Which of the following statements best describes the role of buffers in the food industry?

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